genchem.docx

**lesson 1 - imf** kinetic molecular theory 1. 2. 3. 4. **intermolecular forces** - - - **london dispersion forces** - - - **ion-dipole forces** - - **hydrogen bond** - - **lesson 2 - properties of liquids** **viscosity** - measure of a fluid's resistance t...

**lesson 1 - imf** kinetic molecular theory 1. 2. 3. 4. **intermolecular forces** - - - **london dispersion forces** - - - **ion-dipole forces** - - **hydrogen bond** - - **lesson 2 - properties of liquids** **viscosity** - measure of a fluid's resistance to flow **surface tension** - tendency of fluid to acquire the least possible surface area **boiling point** - temperature at which a substance changes from liquid to gas - **heat of vaporization** - the amount of energy that must be added to a liquid phase in a closed system. substances with stronger imfa have lower vapor pressure compared to those w weaker imfa **lesson 3 - properties of solids** **two general types of solid:** **crystalline** - arranged in fixed geometric patterns or lattices - **amorphous** - have a random orientation of particles - **xray diffraction** - a technique used to determine the atomic and molecular structure of a crystal. **feature of crystalline solids** 1. 2. **molecular crystals -** made of atoms such as in noble gases **covalent network crystals** - made of atoms in which each atom is covalently bonded to is nearest neighbors **lesson 4 - phase diagram** **phase diagram** - describes the phase of a substance at a particular temp and pressure **phase changes** - described as a dynamic equilibria between two opposing physical processes **lesson 5 - heating and cooling** **heating and cooling curves** - used to track heat changes associated with complex phase transformations. - - **lesson 6 - types of solution** - - - - - - - - - most common unit of concentration is **molarity** (M) **mole fraction** - the number of moles of a specific component in the solution divided by the total number of moles in the given solution. []{.math.inline} formulas mole fraction = [\$\\frac{\\text{num\\ of\\ mass}}{\\text{molar\\ mass}}\$]{.math.inline} [\$n\_{a}\\ = \\ \\frac{\\text{mass\\ of\\ solvent}}{\\text{mm\\ of\\ solvent}}\$]{.math.inline} [\$n\_{b}\\ = \\ \\frac{\\text{mass\\ of\\ solute}}{\\text{mm\\ of\\ solute}}\$]{.math.inline} [*n*~*t*~ = *n*~*a*~+ *n*~*b*~]{.math.inline} [\$x\_{a}\\ = \\ \\frac{\\text{moles\\ of\\ solute}}{\\text{moles\\ of\\ solution}}\$]{.math.inline} [\$x\_{b}\\ = \\ \\frac{\\text{moles\\ of\\ solvent}}{\\text{moles\\ of\\ solution}}\$]{.math.inline} molarity = [\$\\frac{\\text{moles\\ of\\ solute}}{\\text{L\\ of\\ solution}}\$]{.math.inline} (M) molality = [\$\\frac{\\text{moles\\ of\\ solute}}{\\text{kg\\ of\\ solvent}}\$]{.math.inline} (m)